Give your answers in this section to three decimal places.
Work out the mass of carbon contained in $0.352\,\text{g}$ of $\text{CO}_2$. Use that result to find the amount, in moles, of carbon atoms in $0.240\,\text{g}$ of A.
Work out the mass of hydrogen present in $0.144\,\text{g}$ of $\text{H}_2\text{O}$. Use that value to calculate the amount, in moles, of hydrogen atoms in $0.240\,\text{g}$ of A.
Use your answers to work out the mass of oxygen in $0.240\,\text{g}$ of A. Use this value to calculate the amount, in moles, of oxygen atoms in $0.240\,\text{g}$ of A.
Use your answers to (a) to determine the empirical formula of A.
A $0.148\,\text{g}$ sample of A was vapourised at $60^{\circ}\text{C}$, and its vapour occupied $67.7\,\text{cm}^3$ at a pressure of $101\,\text{kPa}$.
Use the general gas equation $pV = nRT$ to calculate $M_r$ for A.
From this, calculate the molecular formula of A.
Compound A is a liquid that shows no reaction with 2,4-dinitrophenylhydrazine reagent or with aqueous bromine. Suggest two structural formulae for A.
Compound A contains only carbon, hydrogen and oxygen. Explain how the details on the opposite page about A reacting with $\text{CuO}$ support this statement.